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2 years ago

Calculate the density of a sample of 1.00 mole of NH3 at 793mmHg and -9.00 C

Chemistry

1 answer:

Andrews [41]2 years ago

5 0

Answer:

A mixture of 2.00 moles of H., 3.00 moles of NH3, 4.00 moles of Co, and 5.00 moles.

Explanation:

A mixture of 2.00 moles of H., 3.00 moles of NH3, 4.00 moles of Co, and 5.00 moles.

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Table salt, NaCl, is an example of an amorphous solid. TRUE FALSE

prohojiy [21]

False, it is an example of an Ionic solid

3 0

2 years ago

Read 2 more answers

You are asked to go into the lab and prepare an acetic acid - sodium acetate buffer solution with a ph of 4.00  0.02. what mola

Oxana [17]

Hello!

To solve this problem we are going to use the Henderson-Hasselbach equation and clear for the molar ratio. Keep in mind that we need the value for Acetic Acid's pKa, which can be found in tables and is 4,76:

$pH=pKa + log ( \frac{[CH_3COONa]}{[CH_3COOH]} )$

$\frac{[CH_3COOH]}{[CH_3COONa}= 10^{(pH-pKa)^{-1}}=10^{(4-4,76)^{-1}}=5,75$

So, the mole ratio of CH₃COOH to CH₃COONa is 5,75

Have a nice day!

5 0

2 years ago

A gem has a mass of 4.50 g. When the gem is placed in a graduated cylinder 12.00 mL of water, the water level rises to 13.45 mL.

Mandarinka [93]

Displaced volume :

Final volume - Initial volume

13.45 mL - 12.00 mL => 1.45 mL

Mass = 4.50 g

Therefore:

density = mass / volume

D = 4.50 / 1.45

D = 3.103 g/mL

6 0

2 years ago

A student checks the air in her bicycle tires early in the morning when it is cool outside. If she measures it again later in th

Dmitry_Shevchenko [17]

Answer:

She will observe that the pressure on the tire is higher.

Explanation:

By the ideal gas law, the pressure and the temperature are directly proportional, so, if the temperature increases the pressure increases too:

PV = nRT (P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature).

The temperature is a measure of the average kinetic energy of the gas molecules, so when the temperature increases, the energy also increases, and the gas molecules will move more quickly, so they will collide more often between themselves and in the wall. Those collisions will be with more force because the velocity is higher.

So, the pressure will be higher, because it is the result of collisions of the gas molecules with the walls of the tire.

6 0

2 years ago

According to the equation below, how many moles of Ca(OH)2 are required to react with 1.36 mol H3PO4 to produce Ca3(PO4)2? 3Ca(O

allsm [11]

Answer: The amount of calcium hydroxide needed to react is 2.04 moles

Explanation:

We are given:

Moles of phosphoric acid = 1.36 moles

For the given chemical equation:

$3Ca(OH)_2+2H_3PO_4\rightarrow Ca_3(PO_4)_2+6H_2O$

By Stoichiometry of the reaction:

2 moles of phosphoric acid reacts with 3 moles of calcium hydroxide

So, 1.36 moles of phosphoric acid will react with = $\frac{3}{2}\times 1.36=2.04mol$ of calcium hydroxide

Hence, the amount of calcium hydroxide needed to react is 2.04 moles

3 0

2 years ago