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Trava [24]
2 years ago
10

What is the molar mass of an unknown gas if the density of that gas is 0.726 grams/liter at a pressure of 0.634 atm and a temper

ature of 25oC?
a. 2.35 g/mole
b. 28.0 g/mole
c. 53.2 g/mole
d. 64.0 g/mole
Chemistry
1 answer:
pshichka [43]2 years ago
5 0

Answer:

b. 28.0 g/mole

Explanation:

Given:

d = 0.726 g/L

P = 0.634 atm

T = 25°C + 273 = 298 K

We can use the ideal gas equation of state:

PV= nRT

Since d=mass/V = nM/V, we can modify the equation to obtain the molar mass of the gas (M):

PM = dRT

⇒ M = dRT/P = (0.726 g/L x 0.082 L.atm/K.mol x 298 K)/(0.634 atm)= 27.87 g/mol ≅ 28 g/mol

Therefore, the correct option is b. 28.0 g/mole

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What is the percent composition of phosphoric acid (H3PO4)?
aleksklad [387]

Answer:

H3PO4 Mol mass..

= (3 x H1 = 3) + (1 x P31 = 31) + (4 x O16 = 64). = 98g/mol.

a)..Hydrogen: = 3 / 98 = 0.0306 x 100% = 3.06%.

b)..Phosphorus = 31/98 = 0.3162 x 100% = 31.63%.

c)..Oxygen = 64/98 = 0.6531 x 100% = 65.31%.

(Total = 100% H3PO4).

Explanation:

Find the molar mass of all the elements in the compound in grams per mole.

Find the molecular mass of the entire compound.

Divide the component's molar mass by the entire molecular mass.

You will now have a number between 0 and 1. Multiply it by 100% to get percent composition.

8 0
2 years ago
What would happen to the amount of matter on Earth if mass were not conserved during the changes on states?
Mademuasel [1]
What would happen to the amount of matter on earth if mass were not conserved during changes of state?
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2 years ago
Consider the following redox equation Mn(OH)2(s) + MnO4 –(aq)  MnO42 –(aq) (basic solution) When the equation is balanced with
inysia [295]

Answer : The balanced chemical equation is,

2MnO_4^-(aq)+Mn(OH)_2(s)+4OH^-(aq)\rightarrow 3MnO_4^{2-}(aq)+2H_2O(l)

The coefficient for OH^- is, 4 and on reactant side of the equation OH^-(aq) is present.

Explanation :

Rules for the balanced chemical equation in basic solution are :

  • First we have to write into the two half-reactions.
  • Now balance the main atoms in the reaction.
  • Now balance the hydrogen and oxygen atoms on both the sides of the reaction.
  • If the oxygen atoms are not balanced on both the sides then adding water molecules at that side where the more number of oxygen are present.
  • If the hydrogen atoms are not balanced on both the sides then adding hydroxide ion (OH^-) at that side where the less number of hydrogen are present.
  • Now balance the charge.

The half reactions in the basic solution are :

Reduction : Mn(OH)_2(s)+1e^-\rightarrow MnO_4^{2-}(aq) ......(1)

Oxidation : MnO_4^-(aq)+4OH^-(aq)\rightarrow MnO_4^{2-}(aq)+2H_2O(l)+2e^-.....(2)

Now multiply the equation (1) by 2 and then added both equation, we get the balanced redox reaction.

The balanced chemical equation in a basic solution will be,

2MnO_4^-(aq)+Mn(OH)_2(s)+4OH^-(aq)\rightarrow 3MnO_4^{2-}(aq)+2H_2O(l)

Thus, the coefficient for OH^- is, 4 and on reactant side of the equation OH^-(aq) is present.

6 0
2 years ago
A student places 1.38g of unknown metal at 99.6C into 60.50g of water at 22.1C. The entire system reaches a uniform temperature
stiv31 [10]

Explanation:

Heat energy lost by metal = Heat energy gained by water.

(0.00138kg) * c * (99.6-31.6) = (0.006050kg) * 4.148 * (31.6-22.1)

c = 2.541J/kg°C

8 0
3 years ago
The Ksp for Cu(OH)2 is 4.8 × 10-20. Determine the molar solubility of Cu(OH)2 in a buffer solution with a pH of 10.1.
Papessa [141]

Answer:

E) 3.0x10⁻¹²

Explanation:

Ksp of Cu(OH)₂ is defined as:

Cu(OH)₂(s) ⇄ Cu²⁺(aq) + 2 OH⁻(aq)

Ksp = [Cu²⁺] [OH⁻]²

When pH is 10.1,  [OH⁻] is:

pOH = 14 - pH

pOH = 3.9

pOH = -log [OH⁻]

<em>[OH⁻] = 1.26x10⁻⁴M</em>

<em />

Replacing in ksp formula:

4.8x10⁻²⁰= [Cu²⁺] [1.26x10⁻⁴]²

<em>3.0x10⁻¹² = [Cu²⁺] </em>

That means the maximum amount of Cu²⁺ that can be in solution is 3.0x10⁻¹²M, thus, molar solubility of Cu(OH)₂ is

<em>E) 3.0x10⁻¹²</em>

3 0
3 years ago
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