Question

a chemistry mixes 108g of H2O with 186L if NO2 at STP. How many grams of NO will be produced?

Answer 1

Do you still need help with this question? @danajohnson29

Answer 2

Yes

Answer 3

Can you help me with the answer? I’m trying to help my son with this. Thanks

Answer 4

@vocaloid could you help with this question and the one right above it?

Answer 5

This is a multistep problem, and here is an outline for how to approach it. You need a few things here.
1. Formulate the balanced chemical equation for H2O+NO2->NO to determine the stoichiometric ratio (how many moles of NO are produced). You don't technically need the balanced chemical equation, but you will need to know what the ratio of reactants to products is and which reactant is limiting (as this will determine the qmaount of product you have)
2. At STP, 1 mole of ideal gas occupies 22.4L. This follows from the ideal gas law and ideal gas constant. (Use this to go from L of NO2 to moles)
3 . You need to calculate molar masses of your reactants and products and (go from moles of NO and NO2 to grams). In other words, use the periodic table to determine the g/mol of each of the relevant reactants and products and convert units from moles to grams.

Answer 6

still need the aswer?