Answer:
pH = 9.25
Explanation:
Reaction of ammonia (NH₃) with hydrochloric acid (HCl) is:
NH₃ + HCl → NH₄⁺ + Cl⁻
As equal volumes of a 0.020M solution of NH₃ and a 0.010M solution of react, molarity of NH₃ after reaction is 0.010M and 0.010M of NH₄⁺.
For the buffer NH₄⁺/NH₃ H-H equation to find pH of solution is:
pH = pKa + log₁₀ [NH₃] / [NH₄⁺]
pH = 9.25 + log₁₀ [0.010M] / [0.010M]
<em>pH = 9.25</em>
<span>The molar mass of the Formaldehyde is about 30 gram per mol which means it goes like 90/30 =3.
So, the molecular formula would be 3 times the empirical formula. C3H6O3.</span>
2 C4H8O + 11 O2 —> 8 CO2 + 8 H2O
its density should stay the same as it is a characteristic property and nothing was added sooo
Answer:
50.00 g of NO
Explanation:
Remember that the balanced chemical reaction equation is indispensable in solving any question that has to do with stoichiometry. Hence the first step in solving the problem is noting down the balanced chemical reaction equation.
2NO(g) + O2 (g)→ 2NO2(g)
Now we try to find out the reactant in excess. The reactant in excess gives the greater mass of product.
For O2;
From the balanced reaction equation;
32 g of O2 yields 92g of NO2
16.00g of O2 will yield 16.00×92/32 = 46g of NO2
For NO;
30g of NO yields 92g of NO2
80.00 g of NO yields 80.00 × 92/30 = 245.33 g of NO2
Hence NO is the reactant in excess.
If 1 mole of O2 reacts with 2 moles of NO2 according to the balanced reaction equation
Then 32 g of O2 reacts with 60g of NO according to the balanced reaction equation
16.00 g of O2 reacts with 16.00 × 60 /32 = 30 g of NO
Hence mass of excess reactant used in the reaction = total mass of NO- mass of NO reacted= 80.00g -30.00g = 50.00 g of NO
Hence the mass of excess reactant used in the reaction is 50.00 g of NO