If 45.5 g of calcium carbonate is reacted with phosphoric acid, how many grams of carbon dioxide will be produced if the reaction yield is 85.0 %?
1. 2.017 moles of Ba(NO3)2 is equivalent to how many grams of NO3-?
N = 14 g/mol
O3 = 3*16 = 48 g/mol
so
NO3 is 62 g/mol
so
(NO3)2 is 124 g/mol
1.2017 * 124 =
To determine the grams of carbon dioxide (CO2) produced, we need to consider the reaction between calcium carbonate (CaCO3) and phosphoric acid (H3PO4). The balanced chemical equation for this reaction is:
3CaCO3 + 2H3PO4 → Ca3(PO4)2 + 3CO2 + 3H2O
From the equation, we can see that for every 3 moles of CaCO3 reacted, 3 moles of CO2 are produced. To calculate the theoretical yield of CO2, we need to convert the given mass of CaCO3 (45.5 g) to moles using its molar mass.
The molar mass of CaCO3 can be calculated as follows:
- Atomic mass of Ca: 40.08 g/mol
- Atomic mass of C: 12.01 g/mol
- Atomic mass of O: 16.00 g/mol (there are 3 oxygen atoms in CaCO3)
Therefore,
Molar mass of CaCO3 = (40.08 g/mol) + (12.01 g/mol) + (16.00 g/mol × 3) = 100.09 g/mol
Converting the mass of CaCO3 to moles:
45.5 g CaCO3 × (1 mol CaCO3 / 100.09 g CaCO3) = 0.454 mol CaCO3
Since the balanced equation shows that 3 moles of CaCO3 produce 3 moles of CO2, we can determine the moles of CO2 produced using stoichiometry.
Therefore, the theoretical yield of CO2 is 0.454 mol CO2.
To find the grams of CO2 produced, we need to convert moles to grams using the molar mass of CO2.
The molar mass of CO2 can be calculated as follows:
- Atomic mass of C: 12.01 g/mol
- Atomic mass of O: 16.00 g/mol (there are 2 oxygen atoms in CO2)
Therefore,
Molar mass of CO2 = 12.01 g/mol + (16.00 g/mol × 2) = 44.01 g/mol
Converting the moles of CO2 to grams:
0.454 mol CO2 × (44.01 g CO2 / 1 mol CO2) = 19.96 g CO2
However, the question mentions that the reaction yield is 85.0%. The reaction yield represents the actual amount of product obtained relative to the theoretical yield. To calculate the actual yield of CO2, we multiply the theoretical yield by the percent yield.
Actual yield of CO2 = 19.96 g CO2 × (85.0 / 100) = 16.97 g CO2
Therefore, if 45.5 g of calcium carbonate is reacted with phosphoric acid with a reaction yield of 85.0%, approximately 16.97 g of carbon dioxide will be produced.