Consider the following balanced equation.
2 H2 + O2 ---> 2 H2O
Which of the following statements is false?
a) One molecule of O2 will react with 2 molecules of H2
b) One mole of O2 will react with 2 moles of H2
c) The complete reaction of 32.0 g of O2 will produce 2 moles of H2O
d) The complete reaction of 2.0 g of H2 will produce 36.0 g of H2O
e) The amount of reaction that consumes 32.0 of g O2 produces of 36.0 g H2O
At first glance, I would think all of these would be right, but obviously that can't be true. But I do know for a fact a and b are both true at least.
LETTER D IS TRUE. Why?
2g of H2 + 1g of O2 --> 36g of H20
Meaning:
2 (1.008g/mol × 2 mol) + 1 (16.0g/mol × 2) = 4.008g + 32g = 36g of H20.
Bobs answer is correct.
Well, well, well, looks like we have a balanced equation on our hands! And some statements to assess, eh? Let's dive in and find the false one, shall we?
Statement a) One molecule of O2 will react with 2 molecules of H2. Ah, the good old stoichiometry! That's absolutely true! O2 and H2, taking a double-date and forming a beautiful H2O.
Statement b) One mole of O2 will react with 2 moles of H2. Aha, just an extension of the previous statement! Absolutely true again. Moles are like friendly numbers that allow us to keep track of how many molecules we have around.
Now, let's move to Statement c) The complete reaction of 32.0 g of O2 will produce 2 moles of H2O. Hmmm, hold your horses there! We need to do some quick calculations. The molar mass of O2 is approximately 32 g/mol. So, 32.0 g of O2 corresponds to 1 mole of O2, not 2 moles. Sorry, Statement c), but you're the clown of the bunch!
But wait, we're not done yet! Let's have a look at Statement d) The complete reaction of 2.0 g of H2 will produce 36.0 g of H2O. Hmmm, let's crunch some numbers, shall we? The molar mass of H2 is approximately 2 g/mol. So, 2.0 g of H2 corresponds to 1 mole of H2, and since we produce 2 moles of H2O, it would be 36.0 g of H2O, not 2.0 g. Oops, it seems Statement d) is also walking the tightrope of falsehood!
Finally, we reach Statement e) The amount of reaction that consumes 32.0 g of O2 produces 36.0 g H2O. Well, now that I've already told you regarding Statement c), you can guess that this one is true! Combining some quick calculations and stoichiometry, we find that 32.0 g of O2 will indeed produce 36.0 g of H2O.
So, my friend, the false statement is c) The complete reaction of 32.0 g of O2 will produce 2 moles of H2O. It seems that one got a bit confused with the mole ratio. Better luck next time, Statement c)!
To determine the false statement among the given options, let's break down each statement and analyze them one by one.
a) One molecule of O2 will react with 2 molecules of H2
This statement is true because the balanced equation shows that 2 molecules of H2 react with 1 molecule of O2.
b) One mole of O2 will react with 2 moles of H2
This statement is also true. The balanced equation indicates that for every 1 mole of O2, 2 moles of H2 react.
c) The complete reaction of 32.0 g of O2 will produce 2 moles of H2O
To determine if this statement is true, we need to calculate the number of moles of O2 in 32.0 g using its molar mass. Oxygen (O2) has a molar mass of approximately 32.0 g/mol. Thus, the number of moles of O2 can be calculated as follows:
moles of O2 = mass of O2 / molar mass of O2
= 32.0 g / 32.0 g/mol
= 1.0 mol
Since 1 mole of O2 produces 2 moles of H2O according to the balanced equation, this statement is false. The complete reaction of 32.0 g of O2 will produce 2 moles of H2O, not 2 moles of H2O.
d) The complete reaction of 2.0 g of H2 will produce 36.0 g of H2O
To check the validity of this statement, we need to determine the number of moles of H2 in 2.0 g using its molar mass. Hydrogen gas (H2) has a molar mass of approximately 2.0 g/mol. So, the number of moles of H2 can be calculated as follows:
moles of H2 = mass of H2 / molar mass of H2
= 2.0 g / 2.0 g/mol
= 1.0 mol
Since 1 mole of H2 reacts to produce 36.0 g of H2O, this statement is false. The complete reaction of 2.0 g of H2 will not produce 36.0 g of H2O.
e) The amount of reaction that consumes 32.0 g of O2 produces 36.0 g of H2O
This statement is also false because the balanced equation shows that 2 moles of H2O are produced when 1 mole of O2 reacts. The molar mass of O2 is approximately 32.0 g/mol, so the amount of O2 required to produce 36.0 g of H2O would be more than 32.0 g.
Therefore, the false statement among the given options is c) The complete reaction of 32.0 g of O2 will produce 2 moles of H2O.