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yanalaym [24]
3 years ago
10

Anouk does 150 J of work using a hammer to pull a nail out of a piece of wood, and the hammer does 105 J of work on the nail. Wh

at is the efficiency of the hammer? 1.4% 7% 70% 143%
Chemistry
2 answers:
Anna35 [415]3 years ago
6 0

Answer:

70%

Explanation:

105 divided by 150 equal to 0.7.  then u multiply 0.7 by 100. equal 70.  so its C because efficiency = (effective work)/(executed work) * 100%

Lesechka [4]3 years ago
5 0

Answer:

70%

Explanation:

105 divided by 150 equal to 0.7.  then u multiply 0.7 by 100. equal 70.  so its C because efficiency = (effective work)/(executed work) * 100%

hope it helped :3

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Write a balanced chemical equation for the photosynthesis reaction in which gaseous carbon dioxide and liquid water react in the
sasho [114]
6 CO₂ + 6 H₂O (chlorophyll + sunlight) ⇒ C₆H₁₂O₆ + 6 O₂ 
the reaction takes place in presence of sunlight and chlorophyll .. 
CO₂ is oxidized and forms Glucose . And oxygen is evolved in this process. 

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2 years ago
(ii) When shale gas is burned, the hydrogen sulfide reacts with oxygen.
Elenna [48]

Answer:

See explanation

Explanation:

Now , we have the equation of the reaction as;

2H2S(g) + 302(g)------->2SO2(g) + 2H2O(g)

This equation shows that SO2 gas is produced in the process. Let us recall that this same SO2 gas is the anhydride of H2SO4. This means that it can dissolve in water to form H2SO4

So, when SO2 dissolve in rain droplets, then H2SO4 is formed thereby lowering the pH of rain water. This is acid rain.

4 0
2 years ago
Do parts a, b and c
Leona [35]

Answer:- (a)The pH of the buffer solution is 3.90.

(b) the pH of the solution after addition of HCl would be 3.60.

(c) the pH of the buffer solution after addition of NaOH is 4.32.

Solution:- (a) It is a buffer solution so the pH could easily be calculated using Handerson equation:

pH=Pka+log(\frac{base}{acid})

pKa can be calculated from given Ka value as:

pKa=-logKa

pKa=-log(6.3*10^-^5)

pKa = 4.20

let's plug in the values in the Handerson equation:

pH=4.20+log(\frac{0.025}{0.05})

pH = 4.20 - 0.30

pH = 3.90

The pH of the buffer solution is 3.90.

(b) Let's say the acid is represented by HA and the base is represented by A^- .

Original mili moles of HA from part a = 0.05(100) = 5

original mili moles of A^- from part a = 0.025(100) = 2.5

mili moles of HCl that is H^+ added = 0.100(10.0) = 1

This HCl reacts with the base present in the buffer to make HA as:

A^-+H^+\rightarrow HA

Total mili moles of HA after addition of HCl = 5+1 = 6

mili moles of base after addition of HCl = 2.5-1 = 1.5

Let's plug in the values in the Handerson equation again. Here, we could use the mili moles to calculate the pH. The answer remains same even if we use the concentrations also as the final volume is same both for acid and base.

pH=4.20+log(\frac{1.5}{6})

pH = 4.20 - 0.60

pH = 3.60

So, the pH of the solution after addition of HCl would be 3.60.

(c) mili moles of NaOH or OH^- added to the original buffer = 0.05(15.0) = 0.75

This OH^- reacts with HA to form A^- as:

HA+OH^-\rightarrow H_2O+A^-

mili moles of HA after addition of NaOH = 5-0.75 = 4.25

mili moles of A^- after addition of NaOH = 2.5+0.75 = 3.25

Let's plug in the values again in Handerson equation:

pH=4.20+log(\frac{3.25}{4.25})

pH = 4.20 - 0.12

pH = 4.32

So, the pH of the buffer solution after addition of NaOH is 4.32.

7 0
2 years ago
In a calorimeter, 10.0 g of ice melts at 0oC. The enthalpy of fusion of the ice is 334 J/g.
d1i1m1o1n [39]

Answer:

D

Explanation:

In the problem above it is

q = mass x heat fusion

q = 10 g x 334 J/g = 3340 J. Since the ice is absorbing heat it is + 334 J.

5 0
2 years ago
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