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frutty [35]
3 years ago
10

What is the volume of 10 paper clips in ml

Chemistry
2 answers:
vredina [299]3 years ago
7 0

Answer:

10.000

Explanation:

Burka [1]3 years ago
4 0
The answer is 10 ml for the volume of the paper clips
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Which of these reactions are redox reactions and why?
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It will be number 1.
NO loses oxygen ie its being reduced to N2
NH3 gains oxygen atom ie its being oxidised to H2O
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3 years ago
If 50. 75 g of a gas occupies 10. 0 l at stp, 129. 3 g of the gas will occupy ________ l at stp.
NeX [460]

22.4L

of any gas contains 1 mol of that gas.

50.75g/10L*22.4L/1 mol= 113.68g/mol- this is the mole weight of your gas

1 mol/113.68g*129.3g=1.137403 mol

Set up a ratio

1.137403mol/x L=1 mol/22.4 L

X=25.477827L, or with sig figs, x=25.5L

8 0
2 years ago
Which of the following statements is true with regard to transverse and longitudinal waves?
Ipatiy [6.2K]

Answer:

D (The last answer)

Explanation:

In a transverse wave, particles oscillate perpendicular to the direction of wave motion.

In a longitudinal wave, the oscillations of particles are parallel to the direction of propagation.

5 0
3 years ago
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An experiment applies heat to a substance and produces a gas that is a new and different substance. Choose the true statement.
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Well if the change is reversible then it is a physical change, but if not then it is a chemical change.
4 0
3 years ago
Suppose the half-life is 9.0 s for a first order reaction and the reactant concentration is 0.0741 M 50.7 s after the reaction s
bazaltina [42]

<u>Answer:</u> The time taken by the reaction is 84.5 seconds

<u>Explanation:</u>

The equation used to calculate half life for first order kinetics:

k=\frac{0.693}{t_{1/2}}

where,

t_{1/2} = half-life of the reaction = 9.0 s

k = rate constant = ?

Putting values in above equation, we get:

k=\frac{0.693}{9}=0.077s^{-1}

Rate law expression for first order kinetics is given by the equation:

k=\frac{2.303}{t}\log\frac{[A_o]}{[A]}     ......(1)

where,

k = rate constant  = 0.077s^{-1}

t = time taken for decay process = 50.7 sec

[A_o] = initial amount of the reactant = ?

[A] = amount left after decay process =  0.0741 M

Putting values in equation 1, we get:

0.077=\frac{2.303}{50.7}\log\frac{[A_o]}{0.0741}

[A_o]=3.67M

Now, calculating the time taken by using equation 1:

[A]=0.0055M

k=0.077s^{-1}

[A_o]=3.67M

Putting values in equation 1, we get:

0.077=\frac{2.303}{t}\log\frac{3.67}{0.0055}\\\\t=84.5s

Hence, the time taken by the reaction is 84.5 seconds

6 0
3 years ago
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