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vazorg [7]
3 years ago
9

A 250.0-ml sample of ammonia, nh3 (g), exerts a pressure of 833 torr at 42.4 °c. what mass of ammonia is in the container

Chemistry
1 answer:
Lelu [443]3 years ago
6 0
To solve this, let's assume ideal gas behavior.

PV=nRT
Let's solve for n. Convert units to SI units first.

Pressure = 833 torr(101325 Pa/760 torr) = 111,057.53 Pa
Volume = 250 mL(1 L/1000 mL)(1 m³/1000 L) = 2.5×10⁻⁴ m³
Temperature = 42.4 + 273 = 315.4 K

n = (8,314 J/mol·K)(315.4 K)/(111057.53 Pa)(2.5×10⁻⁴ m³)
n = 94.45 mol

The molar mass of ammonia is 17.031 g/mol.
Mass = 94.45*17.031 = <em>1,608.51 g ammonia</em>


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Answer:

The turnover number is the maximum substrate quantitiy converted to product per enzyme and per second. It can be calculate as follows:

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it is not like any option.

If we assume that V_{max} have the non usual units of mol L^{-1} min^{-1} and it is 6.8*10^-10 mol min^{-1}

So we need divide by the moles of E (in place of [E])

Now k_c=\frac{6.8*10^-10}{3.38*10^{-14}}=20128 min^{-1} = 335 s{-1}

(pass from min^{-1} to s^{-1} dividing by 60)

4 0
3 years ago
How many grams of ammonium chloride (gram formula mass= 53.5 g) are contained in .500 L of a 2.00 M solution?
Elza [17]

Answer:

53.5g of NH4Cl

Explanation:

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Mole = Molarity x Volume

Mole = 2 x 0.5

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Now, let us convert 1mole of NH4Cl to gram. This is illustrated below:

Molar Mass of NH4Cl = 53.5g/mol

Number of mole = 1

Mass =?

Number of mole = Mass /Molar Mass

Mass = number of mole x molar Mass

Mass = 1 x 53.5

Mass = 53.5g

Therefore, 53.5g of NH4Cl is contained in the solution.

8 0
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eimsori [14]

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Calculate the concentration of the following solution in mol/dm3 0.1 moles of NaCl in 200 cm3
taurus [48]
1 cm ^{3} = 0.001 dm ^{3}. Therefore 200 cm ^{3} = 0.2 dm ^{3}. Molarity = \frac{number of moles of NaCl}{volume of the solution} =  \frac{0.1}{0.2} = 0.5 mol/dm^{3}. Hope this helps.
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