Answer:
53.7 grams of HNO3 will be produced
Explanation:
Step 1: Data given
Mass of NO2 = 59.0 grams
Molar mass NO2 = 46.0 g/mol
Step 2: The balanced equation
3NO2 + H2O→ 2HNO3 + NO
Step 3: Calculate moles NO2
Moles NO2 = 59.0 grams / 46.0 g/mol
Moles NO2 = 1.28 moles
Step 4: Calculate moles HNO3
For 3 moles NO2 we need 1 mol H2O to produce 2 moles HNO3 and 1 mol NO
For 1.28 moles NO2 we'll have 2/3 * 1.28 =0.853 moles HNO3
Step 7: Calculate mass HNO3
Mass HNO3 = 0.853 moles * 63.01 g/mol
Mass HNO3 = 53.7 grams
53.7 grams of HNO3 will be produced
Answer:
Las moléculas de los reactivos tienen que chocar entre sí. Estos choques deben de producirse con energía suficiente de forma que se puedan romper y formar enlaces químicos. En el choque debe haber una orientación adecuada para que los enlaces que se tienen que romper y formar estén a una distancia y posición viable.
Using the stoichiometry of the reaction and the information provided in the question, the mass of N2 used is 11.62 g.
<h3>Chemical reaction</h3>
The term chemical reaction refers to the combiantion of two or substances to yiled one or more products. The reaction equation in this case is N2 + O2 --->2NO.
Now;
Number of moles of NO = 25g/30 g/mol = 0.83 moles
1 mole of N2 yields 2 moles of NO
x moles of N2 yileds 0.83 moles of NO
x = 0.415 moles
Mass of N2 = 0.415 moles * 28 g/mol = 11.62 g
Learn more about stoichiometry:
brainly.com/question/12166462
0.500 moles is roughly .5*6.022*10^23=3.011*10^23 atoms. This is independent of STP.
