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3 years ago

¿Cuántos moles de bióxido de Nitrógeno (NO 2) se forman cuando reaccionan 5 moles de Nitrógeno (N 2)?

Chemistry

1 answer:

o-na [289]3 years ago

5 0

Answer:

10 moles de NO2

Explanation:

Tenemos la ecuación de la reacción como sigue;

N2 (g) + 2 O2 (g) → 2 NO2 (g)

Asi que;

Si 1 mol de nitrógeno produce 2 moles de NO2

5 moles de nitrógeno producirán 5 * 2/1 = 10

Por tanto, se producen 10 moles de NO2 moles

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A gas has a pressure of 450 mmHg at 100 degrees Celsius. What will its new pressure be when the temperature rises 200 degrees Ce

Ahat [919]

Answer:

P2 = 900 mmHg.

Explanation:

Given the following data;

Initial pressure = 450 mmHg

Initial temperature = 100°C

Final temperature = 200°C

To find the final pressure, we would use Gay Lussac's law;

Gay Lussac states that when the volume of an ideal gas is kept constant, the pressure of the gas is directly proportional to the absolute temperature of the gas.

Mathematically, Gay Lussac's law is given by;

$PT = K$

$\frac{P1}{T1} = \frac{P2}{T2}$

Making P2 as the subject formula, we have;

$P_{2}= \frac{P1}{T1} * T_{2}$

$P_{2}= \frac{450}{100} * 200$

$P_{2}= 4.5 * 200$

Final pressure, P2 = 900 mmHg.

3 0

2 years ago

PLEASE HELP! See picture

Darya [45]

Answer:

See Explanation

Explanation:

The equation of the reaction;

KHSO4(aq) + KOH(aq) -------> K2SO4(aq) + H2O(l)

Number of moles of KHSO4 = 49.6 g/136.169 g/mol = 0.36 moles

Since the reaction is in a mole ratio of 1:1, 0.36 moles of K2SO4 is produced.

Number of moles of KOH = 25.3 g/56.1056 g/mol = 0.45 moles

Since the reaction is 1:1, 0.45 moles of K2SO4 is produced

Hence K2SO4 is the limiting reactant.

Mass of K2SO4 formed = 0.36 moles of K2SO4 * 174.26 g/mol = 62.7 g

So;

1 mole of KHSO4 reacts with 1 mole of KOH

0.36 moles of KHSO4 reacts with 0.36 * 1/1 = 0.36 moles of KOH

Amount of excess KOH = 0.45 moles - 0.36 moles = 0.09 moles

Mass of excess KOH = 0.09 moles * 56.1056 g/mol = 5 g of excess KOH

5 0

3 years ago

6. Calculate the molarity if 35.0 grams of KBr are dissolved in 700. ml?

olga55 [171]

Answer:

To calculate molarity, divide the number of moles of solute by the volume of the solution in liters. If you don't know the number of moles of solute but you know the mass, start by finding the molar mass of the solute, which is equal to all of the molar masses of each element in the solution added together.

Explanation:

try starting with 35.0 and dived it by the volume

8 0

3 years ago

Read 2 more answers

What is the value for ∆Soreaction for the following reaction, given the standard entropy values?

Soloha48 [4]

To get the ∆S of the reaction, we simply have to add the ∆S of the reactants and the ∆S of the products. Then, we get the difference between the ∆S of the products and the ∆S of the products. If the ∆S is negative, then the reaction spontaneous. If the otherwise, the reaction is not spontaneous.

8 0

3 years ago

Please help!! i need the answer ASAP!

nirvana33 [79]

Answer:

23.34 %.

Explanation:

The percentage of water must be calculated as a mass percent.

We need to find the mass of water, and the total mass in one mole of the compound. For that we need to use the atomic masses of each element and take in consideration the number of atoms of each element in the formula unit.

Atomic masses of the elements:

Cd: 112.411 g/mol, N: 14.0067 g/mol, O: 15.999 g/mol, and H: 1.008 g/mol.

Mass of the formula unit:

Cd(NO₃)₂•4H₂O

mass of the formula unit = (At. mass of Cd) + 2(At. mass of N) + 10(At. mass of O) + 8(At. mass of H) = (112.411 g/mol) + 2(14.0067 g/mol) + 10(15.999 g/mol) + 8(1.008 g/mol) = 308.5 g/mol.

Mass of water in the formula unit:

mass of water = (4 × 2 × 1.008 g/mol) + (4 × 15.999 g/mol) = 72.0 g/mol.

So, the percent of water in the compound = [mass of water / mass of the formula unit] × 100 = [(72.0 g/mol)/(308.5 g/mol)] × 100 = 23.34 %

7 0

3 years ago