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zvonat [6]
1 year ago
14

Which chemical equations show an oxidation- reduction reaction

Chemistry
1 answer:
saveliy_v [14]1 year ago
4 0

Answer:

 O2 + 2H2 → 2H2O MgSO4 + CaCl2 → MgCl2 + CaSO4 2Al + 6HI → 2AlI3 + 3H2 FeCl2 + Na2CO3 → FeCO3 + 2NaCl 2AgNO3 + Na2S → Ag2S + 2NaNO3

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A gaseous mixture contains 5.0 moles of nitrogen and 10.0 moles of helium . What is the total pressure if the temperature is 25
jolli1 [7]

Answer:

A) 122 atm

Explanation:

PV = nRT

Solve for P --> P = nRT/V

n = 10.0 mol + 5.0 mol = 15.0 mol

R = 0.08206 L atm / mol K

T = 25 + 273 = 298 K

V = 3.0

P = (15.0)(0.08206)(298) / (3.0) = 122 atm

6 0
2 years ago
Given the following UNBALANCED reaction: NH3 (g) <--> N2 (g) + H2 (g) If 1
Yakvenalex [24]

Answer:

C. 1.35

Explanation:

                                                     2NH3 (g) <-->          N2 (g) +             3H2 (g)

Initial concentration                2.2 mol/0.95L       1.1 mol/0.95L           0

change in concentration        2x                             x                           3x

                                                 -0.84 M                  +0.42M                +1.26M

Equilibrium                       1.4 mol/0.95L=1.47M        1.58 M                   1.26 M

concentration

Change in concentration(NH3) = (2.2-1.4)mol/0.95 L = 0.84M

Equilibrium concentration (N2) = 1.1/0.95 +0.42=1.58 M

Equilibrium concentration(NH3) = 1.4/0.95 = 1.47M

K = [N2]*{H2]/[NH3] = 1.58M*1.26M/1.47M = 1.35 M

8 0
2 years ago
Write one benefit of fungi
hichkok12 [17]

Answer:

below

Explanation:

Environmental Benefits. Fungi feed on dead organic matter which includes leaf litter, soil, dung, wood and dead animals.

7 0
3 years ago
An element has an atomic mass number of 16 and an atomic number of 7
Kitty [74]

Answer: Nitrogen

Explanation: Nitrogen has an atomic number of 7 and an atomic mass of about 14 u

7 0
3 years ago
Question 9
Evgesh-ka [11]

Answer:

0.382 atm

Explanation:

In order to find the pressure, you need to know the moles of carbon dioxide (CO₂) gas. This can be found by multiplying the mass (g) by the molar mass (g/mol) of CO₂. It is important to arrange the conversion in a way that allows for the cancellation of units.

Molar Mass (CO₂): 12.011 g/mol + 2(15.998 g/mol)

Molar Mass (CO₂): 44.007 g/mol

15 grams CO₂               1 mole
----------------------  x  ------------------------  =  0.341 moles CO₂
                                44.007 grams

To find the pressure, you need to use the Ideal Gas Law equation.

PV = nRT

In this equation,

-----> P = pressure (atm)

-----> V = volume (L)

-----> n = moles

-----> R = Ideal Gas Constant (0.08206 atm*L/mol*K)

-----> T = temperature (K)

After you convert Celsius to Kelvin, you can plug the given and calculated values into the equation and simplify to find the pressure.

P = ? atm                              R = 0.08206 atm*L/mol*K

V = 20 L                               T = 0 °C + 273.15 = 273.15 K

n = 0.341 moles

PV = nRT

P(20 L) = (0.341 moles)(0.08206 atm*L/mol*K)(273.15 K)

P(20 L) = 7.64016

P = 0.382 atm

7 0
2 years ago
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