a chemist reacts sodium metal and chlorine gas to form salt according to the balanced chemical equation 2na…
a chemist reacts sodium metal and chlorine gas to form salt according to the balanced chemical equation 2na + cl₂ → 2nacl. if the chemist has 35 g na, what mass of chlorine must they use to react completely with the sodium? type in your answer using the correct number of significant figures. 35 g na = g cl₂ done
Answer
Explanation:
Step1: Calculate moles of Na
The molar mass of Na is approximately 22.99 g/mol. The number of moles of Na, $n_{Na}=\frac{m_{Na}}{M_{Na}}$, where $m_{Na} = 35$ g and $M_{Na}=22.99$ g/mol. So $n_{Na}=\frac{35}{22.99}\approx1.522$ mol.
Step2: Determine mole - ratio from the balanced equation
From the balanced equation $2Na + Cl_2\rightarrow2NaCl$, the mole - ratio of $Na$ to $Cl_2$ is 2:1. So the number of moles of $Cl_2$ required, $n_{Cl_2}=\frac{1}{2}n_{Na}$. Substituting $n_{Na} = 1.522$ mol, we get $n_{Cl_2}=\frac{1.522}{2}= 0.761$ mol.
Step3: Calculate mass of $Cl_2$
The molar mass of $Cl_2$ is $M_{Cl_2}=2\times35.45 = 70.90$ g/mol. The mass of $Cl_2$, $m_{Cl_2}=n_{Cl_2}\times M_{Cl_2}$. Substituting $n_{Cl_2}=0.761$ mol and $M_{Cl_2}=70.90$ g/mol, we get $m_{Cl_2}=0.761\times70.90\approx54$ g.
Answer:
54