To determine the number of moles of NaClO3 required to produce 61 moles of O2, we need to use the stoichiometric coefficients from the balanced equation:
2 NaClO3 → 2 NaCl + 3 O2
For every 2 moles of NaClO3, 3 moles of O2 are produced. Therefore, we can set up a proportion:
2 mol NaClO3 / 3 mol O2 = x mol NaClO3 / 61 mol O2
Solving for x, we get:
x = (2/3) * 61 = 40.67
Rounding to the nearest whole number, we get 41 moles of NaClO3.
From the balanced equation:
3 Cu + 8 HNO3 → 3 Cu(NO3)2 + 2 NO + 4 H2O
We can see that for every 8 moles of HNO3, 2 moles of NO are produced. So for 26 moles of HNO3, we can set up a proportion:
8 mol HNO3 / 2 mol NO = 26 mol HNO3 / x mol NO
Solving for x, we get:
x = (2/8) * 26 = 6.5
Therefore, 6.5 moles of NO can be produced.
From the balanced equation:
3 Cu + 8 HNO3 → 3 Cu(NO3)2 + 2 NO + 4 H2O
We can see that for every 8 moles of HNO3, 4 moles of H2O are produced. So for 75 moles of HNO3, we can set up a proportion:
8 mol HNO3 / 4 mol H2O = 75 mol HNO3 / x mol H2O
Solving for x, we get:
x = (4/8) * 75 = 37.5
Therefore, 37.5 moles of H2O can be produced.
Using the stoichiometric coefficients from the balanced equation:
2 NaClO3 → 2 NaCl + 3 O2
We can see that for every 2 moles of NaClO3, 3 moles of O2 are produced. So for 9 moles of NaClO3, we can set up a proportion:
2 mol NaClO3 / 3 mol O2 = 9 mol NaClO3 / x mol O2
Solving for x, we get:
x = (3/2) * 9 = 13.5
Rounding to the nearest whole number, we get 14 moles of O2.
The balanced equation for the reaction is:
C + 2H2 → CH4
The molar mass of methane (CH4) is 12 (from carbon) + 4(1) (from hydrogen) = 16 g/mol.
To find the mass of carbon required to produce 16.1 moles of CH4, we can use the molar ratio between carbon and methane:
1 mol C / 1 mol CH4
Setting up a proportion:
1 mol C / 1 mol CH4 = x mol C / 16.1 mol CH4
Solving for x, we get:
x = 16.1 mol C
Now we need to convert this to grams using the molar mass of carbon, which is 12 g/mol:
16.1 mol C * 12 g/mol = 193.2 g
Therefore, 193