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Georgia [21]
3 years ago
10

Which ones are false? need help please.

Chemistry
2 answers:
konstantin123 [22]3 years ago
7 0

Answer:

False B.)False C.) True D.) False E.) False

Explanation:

kirill [66]3 years ago
5 0

Answer:

A.) False B.)False C.) True D.) False E.) False

Explanation:

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Prejudice

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3 years ago
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Please help me with letter a question
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Rise, decrease, away from ocean, towards land
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Calculate the reaction quotient Qp for the following redox reaction: 14H+ + Cr2O72- + 6Cl- ----> 2Cr3+ + 3Cl2 + 7H2O The reac
stich3 [128]

Answer:

Value of Q_{p} for the given redox reaction is 1.0\times 10^{-8}

Explanation:

Redox reaction with states of species:

14H^{+}(aq.)+Cr_{2}O_{7}^{2-}(aq.)+6Cl^{-}(aq.)\rightarrow 2Cr^{3+}(aq.)+3Cl_{2}(g)+7H_{2}O(l)

Reaction quotient for this redox reaction:

Q_{p}=\frac{[Cr^{3+}]^{2}.P_{Cl_{2}}^{3}}{[H^{+}]^{14}.[Cr_{2}O_{7}^{2-}].[Cl^{-}]^{6}}

Species inside third braket represent concentration in molarity, P represent pressure in atm and concentration of H_{2}O is taken as 1 due to the fact that H_{2}O is a pure liquid.

pH=-log[H^{+}]

So, [H^{+}]=10^{-pH}

Plug in all the given values in the equation of Q_{p}:

Q_{p}=\frac{(0.10)^{2}\times (0.010)^{3}}{(10^{-0.0})^{14}\times (1.0)\times (1.0)^{6}}=1.0\times 10^{-8}

7 0
3 years ago
Which notation represents atoms that have the same number of protons but a different neutron?
ArbitrLikvidat [17]
Those are called isotopes,

the answer is 3.

each element has its own unique number of protons (atomic number) but a different number of neutrons can be shown in example number 3.
5 0
3 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
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