Calculate the number of moles
9.00 g of H2O
88.0 g of CO2
1.70 g of NH3

Answers

Answer 1

Answer: no. of moles -= given mass/ molar mass

1) 9 g of H2O = 9/18 = 1/2 = 0.5 mole

2) 88g of CO2 = 88/44 = 2moles

3) 1.7 g of NH3 = 1.7/17 = 0.1 mole

Answer 2

Answer: number of moles= mass/molar mass
1. 9 g of H2O =9/18=0.5 moles
2.88 gof CO2=88/44=2 moles
3.70 g of NH3=70/17=4.12 moles

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If the hydrogen ion concentration is 10-7M, what is the pH of the solution?Show all work.

Answers

Remember pH=-log(H ions). So it would be pH=-log(10^-7).

A gas sample is at 25°C and 1.0 atmosphere. Which changes in temperature and pressure will cause this sample to behave more like an ideal gas?(1) decreased temperature and increased pressure
(2) decreased temperature and decreased pressure
(3) increased temperature and increased pressure
(4) increased temperature and decreased pressure

Answers

The changes in temperature and pressure will cause this sample to behave more like an ideal gas by increased temperature and decreased pressure. Hence option 4 is correct.

What is ideal gas?

Ideal gas is defined as a gas that physically behaves in accordance with the ideal, or general, gas law, which is a certain idealized relationship between pressure, volume, and temperature. The ideal gas law can be used to calculate the volume of gases that are produced or used. The ideal-gas equation is frequently used in chemical equations to convert between volumes and molar values.

Ideal gases are those that have little volume and no intermolecular forces. Real gas must have intermolecular attractions and volume in order to exist. At low pressure and high temperature, a genuine gas will act as it should.

Thus, the changes in temperature and pressure will cause this sample to behave more like an ideal gas by increased temperature and decreased pressure. Hence option 4 is correct.

To learn more about ideal gas, refer to the link below:

brainly.com/question/28257995

#SPJ2

Answer : The correct option is, (4) increased temperature and decreased pressure

Explanation :

The conditions for ideal gas are, it has no intermolecular attractions and have negligible volume.

The ideal gas equation is,

$PV=nRT$

The conditions for real gas are, it has intermolecular attractions and have volume.

The real gas equation is,

$(P+(an^2)/(V^2))(V-nb)=nRT$

A real gas behave ideally at high temperature and low pressure conditions.

From the given options, option (4) increased temperature and decreased pressure is the correct option.

Hence, increased temperature and decreased pressure this sample to behave more like an ideal gas.

The nitrogenous bases cytosine and thymine area. purines.
b. a phosphate group.
c. a sugar group.
d. pyrimidines.

Answers

Purines are adenine and guanine. So the answer should be D (Pyrimidines). besides, phosphate group and pentose sugar are a part of a nucleotide.

A substance that undergoes radioactive decay is _____ than what it turns into

Answers

...."heavier". *The definition of radioactive decay shall do its explanation.

A solution of ammonia and water contains 1.80×1025 water molecules and 7.00×1024 ammonia molecules. How many total hydrogen atoms are in this solution?

Answers

Answer:

6.40x10²⁵ hydrogen atoms

Explanation:

The solution contains:

1.80x10²⁵ water molecules (H₂O)
7.00x10²⁴ ammonia molecules (NH₄)

We need to calculate the total of hydrogen atoms (H) in the solution.

Each water molecule (H₂O) has 2 hydrogen atoms
Each ammonia molecule (NH₄) has 4 hydrogen atoms

Lets now calculate the number of hydrogen atoms in the solution:

total H atoms = (H atoms in water molecules) + (H atoms in ammonia molecules)

total H atoms = (2 x 1.80x10²⁵) + (4 x 7.00x10²⁴) =

total H atoms = 3.60x10²⁵ + 2.80x10²⁵ = 6.40x10²⁵

1 water molecule contains 2H atoms H atoms in 4.20*10^25 water molecules = 8.4*10^25 H atoms 1 NH3 molecule contains 3 H atoms H atoms in 6.00*10^24 NH3 atoms = 3*6.00*10^24 = 1.8*10^16 H atoms.

Total H atoms = 8.4*10^25 + 1.8*10^25 = 1.02*10^16 H atoms

If 20 atoms of aluminum react with 45 molecules of chlorine gas, which reactant is limiting and how many more atoms/molecules would be required to use up all the reactants?