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PolarNik [594]
4 years ago
14

Explain how the following experimental errors affect the final calculation of the kilocalories per gram for a food item. Be spec

ific as to whether the final value will be higher or lower than if the error had not been made.
a. The student misread the scale and recorded 110.3 g for the final mass of the soda can plus water instead of 101.3 g.
b. Part of the unburned marshmallow fell off before the final mass was determined.
c. The food would not keep burning and had to be relit several times.
d. The thermometer got stuck in the aluminum foil while the food was burning and the final temperature was made with the thermometer in the air above the water and not in the water.
Chemistry
1 answer:
Ainat [17]4 years ago
6 0

Answer:

a) the final kilocalories per gram for food will be less because the mass was reduced

b)the final kilocalories per gram for food will be less since

c) the final kilocalories per gram for food will be less since the reaction will eventually go to completion

d) the final kilocalories per gram for food will be more.

Explanation:

a) the final kilocalories per gram for food will be less because the mass was reduced from 110.3 to 101.3g

b)the final kilocalories per gram for food will be less since some marshmallow fell off before the reaction

c) the final kilocalories per gram for food will be less since the reaction will eventually go to completion

d) the final kilocalories per gram for food will be more since the thermometer that got stuck will add to the value of final kilocalories per gram

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How much energy is required to raise the temperature of 3 kg of iron from 20° C to 25°C? Use the table below and this equation:
ElenaW [278]

The energy required to raise the temperature of 3 kg of iron from 20° C to 25°C is 6,750 J( Option B)

<u>Explanation:</u>

Given:

Specific Heat capacity of Iron= 0.450 J/ g °C

To Find:

Required Energy to raise the Temperature

Formula:

Amount of energy required is given by the formula,

Q = mC (ΔT)

Solution:

M = mass of the iron in g

So 3 kg = 3000 g

C = specific heat of iron = 0.450 J/ g °C [ from the given table]

ΔT = change in temperature = 25° C - 20°C = 5°C

Plugin the values, we will get,

Q = 3000 g ×  0.450 J/ g °C ×  5°C

 = 6,750 J

So the energy required is 6,750 J.

7 0
3 years ago
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What would you expect to observe when you add flour to a glass of water?
algol [13]

Answer:

hmmm

Explanation:

hmmmmmmmmmmmmmmmmmmmmmmmmmmmmmmmmmmmmm

4 0
3 years ago
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How many different compounds are possible, changing only the cis/trans arrangements around these two double bonds?
insens350 [35]
Check the attached file for the answer.

3 0
3 years ago
At 600. K how many moles of gas are in a 1.00 L cylinder at atmospheric pressure?
Anton [14]

Answer:

0.02moles

Explanation:

To answer this question, the general gas law equation is used. The General gas law is:

Pv = nRT

Where; P = standard atmospheric pressure (1 atm)

V = volume (L)

n = number of moles

R = Gas law constant

T = Temperature

For this question; volume = 1.00L, atmospheric pressure (P) = 1 atm, R = 0.0821 L-atm / mol K, T = 600K, n = ?

Therefore; Pv = nRT

n = PV/RT

n = 1 × 1/ 0.0821 × 600

n = 1/49.26

n = 0.0203moles

Hence, there are 0.02 moles of gas.

8 0
3 years ago
Please help me order these bonds
olya-2409 [2.1K]

Answer:

From least polar covalent to most polar covalent;

S-I< Br-Cl < N-H< Te-O

From most ionic to least ionic

Cs-F> Sr-Cl> Li- N> Al-O

Explanation:

Electro negativity is the ability of an atom in a bonding situation to attract the electron pair of a bond towards itself.

Electro negativity difference between two atoms determines the nature of bond existing between any two atoms. When this difference is large, an ionic bond exists in the compound. However, an intermediate difference in electro negativity implies the existence of a polar covalent bond.

Hence, going by electro negativity differences as mentioned in the question, the bonds in the answer were arranged in order of increasing polar covalent nature or decreasing ionic nature as shown.

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3 years ago
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