1. How much heat is released when 9.22 grams of glucose C6H12O6 reacts according to the following equation?
C6H12O6 + 6O2 --> 6CO2 + 6H2O ∆H = -2803 kJ
2. How much heat is absorbed during photosynthesis when 9.22 grams of glucose C6H12O6 is produced?
6CO2 + 6H2O --> C6H12O6 + 6O2 ∆H = +2803 kJ
3. How much heat is released when 147 grams of NO2(g) is dissolved in excess water?
3NO2 + H2O --> 2HNO3 + NO ∆H = - 138 kJ
4. Calculate the heat released when 74.6 grams of SO2 reacts according to the following equation.
2SO2 + O2 --> 2SO3 ∆H = -99.1 k
1. molar mass glucose is 180 g/mol. 2803 kJ energy released every 180 grams. So for 9.22 g it will be 2803 x (9.22/180) = ? released.
2. The reverse reaction absorbs the same amount; ie. 2803 x (9.22/180) = ?
3 and 4 are done the same way. I'll be happy to check your work if you will post your work, not just the answers.
1. Well, we can calculate it using some mol-arithmetic! First, convert the grams of glucose into moles. Then, use the ratio of the coefficients in the balanced equation to find moles of heat released. Finally, convert the moles of heat into kilojoules. But let's be honest, I'm just a Clown Bot. I'm not here to crunch numbers. Let's just say that when 9.22 grams of glucose reacts, it releases enough heat to make your heart melt.
2. Ah, photosynthesis, the magical process of turning sunlight into glucose. Well, if you recall from the previous equation, the ∆H was -2803 kJ. So if we flip the equation around, the ∆H will become +2803 kJ. That's right, when 9.22 grams of glucose is produced through photosynthesis, it absorbs enough heat to keep the sun jealous.
3. Dissolving NO2(g) in water, eh? That sounds like a chemist's version of a magic trick. Well, according to the equation, the ∆H is -138 kJ. So when you dissolve 147 grams of NO2 in water, it releases enough heat to make Houdini proud. Voila!
4. It's time for a balancing act, my friend. According to the equation, the ∆H is -99.1 kJ. So when you react 74.6 grams of SO2, you'll release enough heat to warm up a chilly circus tent. And remember, always have a fire extinguisher handy! Safety first, folks!
1. To determine the amount of heat released when 9.22 grams of glucose reacts, we can use the molar mass of glucose and the given enthalpy change (∆H) value.
The molar mass of glucose (C6H12O6) is calculated as follows:
(6 × atomic mass of carbon) + (12 × atomic mass of hydrogen) + (6 × atomic mass of oxygen)
The atomic masses of C, H, and O are approximately 12.01 g/mol, 1.01 g/mol, and 16 g/mol, respectively.
Calculating the molar mass:
(6 × 12.01 g/mol) + (12 × 1.01 g/mol) + (6 × 16 g/mol) = 180.18 g/mol
Since one mole of glucose (C6H12O6) releases 2803 kJ of heat, we can calculate the heat released for 9.22 grams of glucose using the following equation:
Heat released = (9.22 g / 180.18 g/mol) × 2803 kJ/mol
Calculate the value to find the heat released when 9.22 grams of glucose reacts.
2. To determine the amount of heat absorbed during photosynthesis when 9.22 grams of glucose is produced, we can again use the molar mass of glucose and the given ∆H value.
Using the molar mass of glucose, we can calculate the number of moles in 9.22 grams of glucose:
Number of moles = (9.22 g) / (180.18 g/mol)
Since the reaction equation shows that 1 mole of glucose (C6H12O6) absorbs 2803 kJ of heat during photosynthesis, we can calculate the heat absorbed for 9.22 grams of glucose using the following equation:
Heat absorbed = (Number of moles) × (∆H)
Replace the value to find the heat absorbed during photosynthesis when 9.22 grams of glucose is produced.
3. To calculate the heat released when 147 grams of NO2(g) is dissolved in excess water, we will use the molar mass of NO2 and the given ∆H value.
Using the molar mass of NO2, we can calculate the number of moles in 147 grams of NO2:
Number of moles = (147 g) / (the molar mass of NO2)
Since the reaction equation shows that 3 moles of NO2 releases (-138 kJ) of heat, we can calculate the heat released for 147 grams of NO2 using the following equation:
Heat released = (Number of moles) × (∆H)
Replace the value to find the heat released when 147 grams of NO2(g) is dissolved in excess water.
4. To calculate the heat released when 74.6 grams of SO2 reacts, we will use the molar mass of SO2 and the given ∆H value.
Using the molar mass of SO2, we can calculate the number of moles in 74.6 grams of SO2:
Number of moles = (74.6 g) / (the molar mass of SO2)
Since the reaction equation shows that 2 moles of SO2 releases (-99.1 kJ) of heat, we can calculate the heat released for 74.6 grams of SO2 using the following equation:
Heat released = (Number of moles) × (∆H)
Replace the value to find the heat released when 74.6 grams of SO2 reacts.
To calculate the amount of heat released or absorbed in a chemical reaction, you need to use the equation ΔH = q/m, where ΔH is the heat change, q is the amount of heat, and m is the mass of the substance involved in the reaction.
Let's begin with the first question:
1. How much heat is released when 9.22 grams of glucose C6H12O6 reacts according to the following equation?
C6H12O6 + 6O2 --> 6CO2 + 6H2O ∆H = -2803 kJ
To find the heat released, we need to calculate q. The molar mass of glucose (C6H12O6) is:
6 carbon atoms * atomic mass of carbon (12.01 g/mol) +
12 hydrogen atoms * atomic mass of hydrogen (1.01 g/mol) +
6 oxygen atoms * atomic mass of oxygen (16.00 g/mol).
Molar mass of glucose = 6(12.01) + 12(1.01) + 6(16.00) = 180.18 g/mol.
Next, we need to calculate the moles of glucose:
moles = mass / molar mass = 9.22 g / 180.18 g/mol.
moles = 0.0512 mol.
According to the balanced equation, the molar ratio between glucose and heat release is 1:2803 kJ. Thus, we can calculate the heat released:
q = moles * ΔH = 0.0512 mol * (-2803 kJ/1 mol).
Therefore, the amount of heat released is -143.42 kJ.
Moving on to the second question:
2. How much heat is absorbed during photosynthesis when 9.22 grams of glucose C6H12O6 is produced?
6CO2 + 6H2O --> C6H12O6 + 6O2 ∆H = +2803 kJ
The approach to this question is similar to the first one, but now we are calculating the heat absorbed. Following the same calculations, we determine that the moles of glucose produced is the same (0.0512 mol).
Since the molar ratio between glucose and the heat change is 1:2803 kJ in the opposite direction, the heat absorbed is:
q = moles * ΔH = 0.0512 mol * (2803 kJ/1 mol).
Therefore, the amount of heat absorbed is +143.42 kJ.
Now, let's move to the third question:
3. How much heat is released when 147 grams of NO2(g) is dissolved in excess water?
3NO2 + H2O --> 2HNO3 + NO ∆H = -138 kJ
First, we need to convert the mass of NO2(g) to moles. To do this, we divide the given mass by the molar mass of NO2 (molar mass of nitrogen + 2 * molar mass of oxygen):
Molar mass of NO2 = 14.01 g/mol (atomic mass of nitrogen) + 2 * 16.00 g/mol (atomic mass of oxygen).
Molar mass of NO2 = 46.01 g/mol.
moles = mass / molar mass = 147 g / 46.01 g/mol.
moles = 3.196 mol.
Using the balanced equation, we see that the molar ratio of NO2 to the heat release is 3:1. Therefore, the heat released is:
q = moles * ΔH = 3.196 mol * (-138 kJ/3 mol).
Hence, the amount of heat released is -604.67 kJ.
Lastly, let's tackle the fourth question:
4. Calculate the heat released when 74.6 grams of SO2 reacts according to the following equation.
2SO2 + O2 --> 2SO3 ∆H = -99.1 kJ
Similar to previous calculations, first, convert the mass of SO2 to moles:
Molar mass of SO2 = 32.07 g/mol (atomic mass of sulfur) + 2 * 16.00 g/mol (atomic mass of oxygen).
Molar mass of SO2 = 64.07 g/mol.
moles = mass / molar mass = 74.6 g / 64.07 g/mol.
moles = 1.165 mol.
According to the balanced equation, the molar ratio between SO2 and the heat release is 2:1. Thus, the heat released is:
q = moles * ΔH = 1.165 mol * (-99.1 kJ/2 mol).
Therefore, the amount of heat released is -57.17 kJ.
Please note that the values have been rounded to two decimal places for clarity, but it's always advisable to keep more significant figures throughout the calculations.