Question

1. how many grams of c₂h₂ are produced by adding 5.00 g cac₂?

Explanation:

Step1: Write the chemical reaction equation

$$CaC_{2}+2H_{2}O ightarrow Ca(OH)_{2}+C_{2}H_{2}\uparrow$$

Step2: Calculate the molar mass of \(CaC_{2}\)

The molar mass of \(CaC_{2}\) is \(M_{CaC_{2}}=(40 + 12\times2)\space g/mol=64\space g/mol\)

Step3: Calculate the number of moles of \(CaC_{2}\)

The number of moles of \(CaC_{2}\), \(n_{CaC_{2}}=\frac{m_{CaC_{2}}}{M_{CaC_{2}}}\)
Given \(m_{CaC_{2}} = 5.00\space g\), so \(n_{CaC_{2}}=\frac{5.00\space g}{64\space g/mol}=\frac{5}{64}\space mol\)

Step4: Determine the mole ratio between \(CaC_{2}\) and \(C_{2}H_{2}\)

From the reaction equation, the mole ratio \(n_{CaC_{2}}:n_{C_{2}H_{2}} = 1:1\), so \(n_{C_{2}H_{2}}=n_{CaC_{2}}=\frac{5}{64}\space mol\)

Step5: Calculate the molar mass of \(C_{2}H_{2}\)

The molar mass of \(C_{2}H_{2}\) is \(M_{C_{2}H_{2}}=(12\times2 + 1\times2)\space g/mol = 26\space g/mol\)

Step6: Calculate the mass of \(C_{2}H_{2}\)

The mass of \(C_{2}H_{2}\), \(m_{C_{2}H_{2}}=n_{C_{2}H_{2}}\times M_{C_{2}H_{2}}\)
Substitute \(n_{C_{2}H_{2}}=\frac{5}{64}\space mol\) and \(M_{C_{2}H_{2}} = 26\space g/mol\)
\(m_{C_{2}H_{2}}=\frac{5}{64}\space mol\times26\space g/mol=\frac{130}{64}\space g\approx2.03\space g\)

Answer:

\(2.03\space g\)