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wlad13 [49]
3 years ago
10

2

Chemistry
1 answer:
Katyanochek1 [597]3 years ago
4 0
C because a compound is a substance made of at least two atoms bonded together
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In Na2O, what is the oxidation state of oxygen? In Na2O oxidation state of Na is 1+
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There are millions of organic compounds but only thousands of inorganic compounds because:______
siniylev [52]

Answer:

There are millions of organic compounds but only thousands of inorganic compounds because:

a. organic compounds were formed by living things.

b. there is more carbon on Earth's surface than any other element.

c. atoms of elements other than carbon never combine with themselves.

d. carbon atoms can combine with up to four other atoms, including other carbon atoms.

6 0
1 year ago
Exercise A mixture of 250 mL of methane, CH4, at 35 °C and 0.55 atm and 750 mL of propane, C3Hg, at 35° C and 1.5 atm, were intr
dalvyx [7]

Explanation:

The given data is as follows.

      V_{1} = 250 mL,     V_{2} = 750 mL

      T_{1} = 35^{o}C = 35 + 273 K = 308 K

      T_{2} = 35 + 273 K = 308 K

      P_{1} = 0.55 atm,    P_{2} = 1.5 atm

               P = ? ,         V = 10.0 L

Since, temperature is constant.

So,    P_{1}V_{1} + P_{2}V_{2} = PV

Now, putting the given values into the above formula as follows.

         P_{1}V_{1} + P_{2}V_{2} = PV

         0.55 atm \times 250 mL + 1.5 atm \times 1.5 atm = P \times 10.0 L

                     P = 0.126 atm

As, 1 atm = 760 torr. So, 0.126 atm \times \frac{760 torr}{1 atm} = 95.76 torr.

Thus, we can conclude that the final pressure, in torr, of the mixture is 95.76 torr.

8 0
2 years ago
At 1.00 atmosphere pressure, a certain mass of a gas has a temperature of 100oC. What will be the temperature at 1.13 atmosphere
Inessa [10]

Answer:  Final temperature of the gas will be 330 K.

Explanation:

Gay-Lussac's Law: This law states that pressure is directly proportional to the temperature of the gas at constant volume and number of moles.

P\propto T     (At constant volume and number of moles)

{P_1\times T_1}={P_2\times T_2}

where,

P_1 = initial pressure of gas   = 1.00 atm

P_2 = final pressure of gas  = 1.13 atm

T_1 = initial temperature of gas  = 100^0C=(100+273)K=373K K

T_2 = final temperature of gas  = ?

{1.00\times 373}={1.13\times T_2}

T_2=330K

Therefore, the final temperature of the gas will be 330 K.

7 0
3 years ago
For a reaction Y → X with a very high equilibrium constant, K, which of the following is true? You can refer to the following tw
Dafna11 [192]

Answer:The amount of product will be higher than the amount of substrate at equilibrium

Explanation:

Recall that the equilibrium constant K depends on the amounts of reactants and products present in the system at equilibrium.

Considering the equation; K = [X]/[Y], as the concentration of X increases above that of Y, the equilibrium constant K becomes very high, hence the answer above.

8 0
3 years ago
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