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qaws [65]
2 years ago
7

An excess of mg(s) is added to 100.ml of 0.400 m hcl. at 0c and 1 atm pressure, what volume of h 2 (g) can be obtained?

Chemistry
1 answer:
ra1l [238]2 years ago
5 0
The balanced equation for the reaction between Mg and HCl is as follows
Mg + 2HCl --> MgCl₂ + H₂
stoichiometry of HCl to H₂ is 2:1

number of HCl moles reacted - 0.400 mol/L x 0.100 L = 0.04 mol of HCl
since Mg is in excess HCl is the limiting reactant 
number of H₂ moles formed - 0.04/2 = 0.02 mol of H₂

we can use ideal gas law equation to find the volume of H₂
PV = nRT 
where 
P - pressure - 1 atm x 101 325 Pa/atm = 101 325 Pa
V - volume
n - number of moles - 0.02 mol
R - universal gas constant - 8.314 Jmol⁻¹K⁻¹
T - temperature in Kelvin - 0 °C + 273 = 273 K
substituting these values in the equation 

101 325 Pa x V = 0.02 mol x 8.314 Jmol⁻¹K⁻¹ x 273 K
V = 448 x 10⁻⁶ m³
V = 448 mL 
therefore answer is 
c. 448 mL 
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Answer:

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    |

Br-P-Br

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Explanation:

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4 0
2 years ago
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Explanation:

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3 years ago
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Urea, (NH2)2CO, is a product of metabolism of proteins. An aqueous solution is 37.2% urea by mass and has a density of 1.032 g/m
Feliz [49]

Answer:

The molarity of urea in this solution is 6.39 M.

Explanation:

Molarity (M) is <em>the number of moles of solute in 1 L of solution</em>;  that is

molarity = moles of solute ÷ liters of solution

To calculate the molality, we need to know the number of moles of urea and the volume of solution in liters. We assume 100 grams of solution.

Our first step is to calculate the moles of urea in 100 grams of the solution,

using the molar mass a conversion factor. The total moles of 100g of a 37.2 percent by mass solution is

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Now we need to calculate the volume of 100 grams of solution, and we use density as a conversion factor.

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This solution contains 0.619 moles of urea in 96.9 mL of solution. To express it in molarity, we need to calculate the moles present in 1000 mL (1 L) of the solution.

0.619 mol/96.9 mL × 1000 mL= 6.39 M

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3 years ago
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I NEED HELP ASAP!!!
Rus_ich [418]

Explanation:

To answer this question, we'll need to use the Ideal Gas Law:

p

V

=

n

R

T

,

where

p

is pressure,

V

is volume,

n

is the number of moles

R

is the gas constant, and

T

is temperature in Kelvin.

The question already gives us the values for

p

and

T

, because helium is at STP. This means that temperature is

273.15 K

and pressure is

1 atm

.

We also already know the gas constant. In our case, we'll use the value of

0.08206 L atm/K mol

since these units fit the units of our given values the best.

We can find the value for

n

by dividing the mass of helium gas by its molar mass:

n

=

number of moles

=

mass of sample

molar mass

=

6.00 g

4.00 g/mol

=

1.50 mol

Now, we can just plug all of these values in and solve for

V

:

p

V

=

n

R

T

V

=

n

R

T

p

=

1.50 mol

×

0.08206 L atm/K mol

×

273.15 K

1 atm

= 33.6 L

this is not the answer but it will help you

do by the formula it is on the answer

3 0
2 years ago
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