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muminat
3 years ago
6

Which of the following is true about neutrons?

Chemistry
1 answer:
Alja [10]3 years ago
5 0
D is the only choice here that is appropriate given neutrons' lack of charge
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1 C3H8 + 5 O2 --> 3 CO2 + 4H20. If 1.5 moles of C3H8 react, how many
UNO [17]

Answer:

First confirm the reaction is balanced:

C3H8 + 5O2 --> 3CO2 + 4H20 (3 cabon - check; 8 hydrogen - check; 10 oxygen - check).

a) In the equation there is a 5:1 ratio between propane and oxygen.  We also know that number of mole is proportional to pressure and volume.  Since pressure is constant (STP) then the volume of O2 is 7.2 * 5 = 36 litres.

b) For a near ideal gas that PV = nRT (combined gas law).  So for 7.2 litres propane we find n(propane) = 101.3 * 7.2/8.314*298 ~ 0.29 mole (using metric units throughout for simplicity).

There is a 1:3 ratio between propane and CO2.  Therefore 3 * 0.29 = 0.87 mole of CO2 is produced.

MW(CO2) ~ 44 g/mol.  Therefore m(CO2) = 44 * 0.87 ~ 38.3 g

c) We know we need more oxygen than propane (due to the 1:5 ratio) so oxygen is the limiting reagent.  Again Volume is proportional to number of mole and we see there is a 5:4 ratio between oxygen and water.  Therefore the volume of water vapour produced will be (4/5) * 15 = 12 litres.

The other questions use the same technique and will give you some much needed practice.

Explanation:

7 0
3 years ago
How would a solution that is labeled 5.0 M would be read as?
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5 moles because molarity signifies number of moles dissolved in One litre of water
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The colour imparted to a flame by calcium ion?
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The flame goes an Orange-Red colour.
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What are 3 types of mutations
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1- Base substitutions.

2- Deletions.

3- Insertions.

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The elementary reaction 2H2O(g)↽−−⇀2H2(g)+O2(g) 2H2O(g)↽−−⇀2H2(g)+O2(g) proceeds at a certain temperature until the partial pres
Dima020 [189]

Answer:

6.25\times 10^{-6} is the value of the equilibrium constant at this temperature.

Explanation:

Equilibrium constant in terms of partial pressure is defined as the ratio of partial pressures of products to the partial pressures  of reactants each raised to the power equal to their stoichiometric ratios. It is expressed as K_{p}

2H_2O(g)\rightleftharpoons 2H_2(g)+O_2(g)

Partial pressures at equilibrium:

p^o_{H_2O}=0.070 atm

p^o_{H_2}=0.0035 atm

p^o_{O_2}=0.0025 atm

The equilibrium constant in terms of pressures is given as:

K_p=\frac{(p^o_{H_2})^2\times (p^o_{O_2})}{(p^o_{H_2O})62}

K_p=\frac{(0.0035 atm)^2\times 0.0025 atm}{(0.070 atm)^2}=6.25\times 10^{-6}

6.25\times 10^{-6} is the value of the equilibrium constant at this temperature.

5 0
3 years ago
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