Examine the following unbalanced equation.
HCl (g) + O2 Cl2 (g) + H2O (g)

Assuming that all the gases in this reaction are at STP, what number of molecules of hydrogen chloride gas are needed to completely react with oxygen to yield 50.00 mL of chlorine gas?

Question

Examine the following unbalanced equation.
HCl (g) + O2  Cl2 (g) + H2O (g)

Assuming that all the gases in this reaction are at STP, what number of molecules of hydrogen chloride gas are needed to completely react with oxygen to yield 50.00 mL of chlorine gas?

.sam. · Answer

First you need to balance the equation

.sam. · Answer

$$\begin{array}{cc} 4 & \text{H}\text{Cl} \\end{array}\text{ + }\begin{array}{c} \text{O}_2 \\end{array}\text{    $\longrightarrow $    }\begin{array}{cc} 2 & \text{Cl}_2 \\end{array}\text{ + }\begin{array}{cc} 2 & \text{H}_2\text{O} \\end{array}$$

.sam. · Answer

$$50ml=0.050L=0.05dm^3$$

.sam. · Answer

$$0.05dm^3Cl_2\times \frac{1molCl_2}{24dm^3Cl_2}\times\frac{4molHCl}{2molCl_2}\times \frac{2(6.02\times10^{23})moleculesHCl}{1molHCl}=?$$

anonymous · Answer

is the answer 599*10^24 molecules?