An unknown amount of Na(s) is reacted with an excess of NaH2PO4 to produce hydrogen gas and sodium phosphate. The hydrogen gas was captured and compressed into a rigid 150.0mL container which read 10.2atm at 293.1K. How many grams of Na(s) were in the original sample?
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Explanation:
pv=nrt
pv/rt =n
10.2*0.15 / 0.08026 * 20.1=n
n=0.95
equivalent of h2 gas = equivalent reacted na
0.95*2 = moles*1
1.9=moles
w/23=1.9
w=43.7
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