If a 1.58g sample of C2H3X3(g) has a volume of 297mL at 769mm Hg and 35 degrees C. Identify the element X.
A hydrocarbon is burnt completely in air to form 17.6g of carbon dioxide gas and 7.2g of water. Given that the relative atomic mass of C=12,H=1,O=16
equation: $\ce{2NF3(g) +3H2(g) ->N2(g) +6HF(g)}$ In order to produce 0.48 moles of HF(g), How many moles of NF3 would be consumed?
If a 1.58g sample of C2H3X3(g) has a volume of 297mL at 769mm Hg and 35 degrees C. Identify the element X.
A hydrocarbon is burnt completely in air to form 17.6g of carbon dioxide gas and 7.2g of water.
Given that the relative atomic mass of C=12,H=1,O=16
equation: $\ce{2NF3(g) +3H2(g) ->N2(g) +6HF(g)}$
In order to produce 0.48 moles of HF(g), How many moles of NF3 would be consumed?
