If 25 grams of propane burns and the percent yield is 75% how many grams of carbon dioxide is produced? C3H3 + 5O2 —> 4H2O + 3CO2

57 g

Explanation:

Step 1: Write the balanced equation

C₃H₈ + 5 O₂ ⇒ 4 H₂O + 3 CO₂

Step 2: Calculate the mass corresponding to 25 g of propane

The molar mass of C₃H₈ is 44.1 g/mol.

25 g × 1 mol/44.1 g = 0.57 mol

Step 3: Calculate the theoretical yield of CO₂ from 0.57 moles of C₃H₈

The molar ratio of C₃H₈ to CO₂ is 1:3. The theoretical yield of CO₂ is 3/1 × 0.57 mol = 1.7 mol

Step 4: Calculate the real yield of CO₂

We will use the following expression.

real yield = theoretical yield × percent yield

real yield = 1.7 mol × 75%

real yield = 1.3 mol

Step 5: Calculate the mass corresponding to 1.3 moles of carbon dioxide

The molar mass of CO₂ is 44.01 g/mol.

1.3 mol × 44.01 g/mol = 57 g

answer

fusion: the energy source of stars. the energy released from the collapse of the gas into a protostar causes the center of the protostar to become extremely hot. when the core is hot enough, nuclear fusion commences. fusion is the process where two hydrogen atoms combine to form a helium atom, releasing energy.

hope it

the answer would be c