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3 years ago

What is the mass in grams of 4.91 moles of ammonium sulfate?

Chemistry

2 answers:

Montano1993 [528]3 years ago

4 0

1 mole is equal to 1 moles Ammonium Sulfate, or 132.13952 grams

Strike441 [17]3 years ago

4 0

Answer:

648.12g

Explanation:

First, we need to find the molar mass of ammonium sulphate (NH4)2SO4. This can be achieved by:

Molar Mass of (NH4)2SO4 = 2(14+4)+32+(4x16) = 132g/mol

Mass of (NH4)2SO4 = 4.91x132 = 648.12g

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Use the definition of molarity to calculate the concentration of 12.34 g of CaSO4 completely dissolved in water, with a solution

Ede4ka [16]

Answer:

[CaSO₄] = 36.26×10⁻² mol/L

Explanation:

Molarity (M) → mol/L → moles of solute in 1L of solution

Let's convert the volume from mL to L

250 mL . 1L/1000 mL = 0.250L

We need to determine the moles of solute. (mass / molar mass)

12.34 g / 136.13 g/mol = 0.0906 mol

M → 0.0906 mol / 0.250L = 36.26×10⁻² mol/L

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3 years ago

A recipe for spaghetti sauce requires 2.5 cups of tomato sauce. If only metric measures are available, how many milliliters of t

dsp73

Answer: 2.5 cups of tomato sauce is 625 milliliters of tomato sauce

Explanation:

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2 years ago

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8_murik_8 [283]

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7 0

3 years ago

Read 2 more answers

What is the ph of a solution of 0.550 m k2hpo4, potassium hydrogen phosphate?

Solnce55 [7]

We assume that we have Ka= 4.2x10^-13 (missing in the question)
and when we have this equation:
H2PO4 (-) → H+ + HPO4-
and form the Ka equation we can get [H+]:
Ka= [H+] [HPO4-] / [H2PO4] and we have Ka= 4.2x10^-13 & [H2PO4-] = 0.55m
by substitution:
4.2x10^-13 = (z)(z)/ 0.55
z^2 = 2.31x 10^-13
z= 4.81x10^-7
∴[H+] = 4.81x10^-7
when PH equation is:

PH= -㏒[H+]
= -㏒(4.81x10^-7) = 6.32

3 0

3 years ago

Hydrogen gas was collected by water displacement. what was pressure of the h2 collected if the temperature was 26°c?

Vedmedyk [2.9K]

The ideal gas law may be written as
$p= \frac{\rho R T}{M}$
where
p = pressure
ρ =density
T = temperature
M = molar mass
R = 8.314 J/(mol-K)

For the given problem,
ρ = 0.09 g/L = 0.09 kg/m³
T = 26°C = 26+273 K = 299 K
M = 1.008 g/mol = 1.008 x 10⁻³ kg/mol

Therefore
$p= \frac{(0.09 \, kg/m^{3})*(8.314 \, J/(mol-K))*(299 \, K)}{1.008 \times 10^{-3} \, kg/mol} =2.2195 \times 10^{5} \, Pa$

Note that 1 atm = 101325 Pa
Therefore
p = 2.2195 x 10⁵ Pa
= 221.95 kPa
= (2.295 x 10⁵)/101325 atm
= 2.19 atm

Answer:
2.2195 x 10⁵ Pa (or 221.95 kPa or 2.19 atm)

4 0

3 years ago