Answer: 0.036 J/g°C
Explanation:
The quantity of heat energy (Q) required to raise the temperature of a substance depends on its Mass (M), specific heat capacity (C) and change in temperature (Φ)
Thus, Q = MCΦ
Given that,
Q = 3.42 Kilojoules
[Convert 3.42 kilojoules to joules
If 1 kilojoule = 1000 joules
3.42 kilojoules = 3.42 x 1000 = 3420J]
Mass = 2.508Kg
[Convert 2.508 kg to grams
If 1 kg = 1000 grams
2.508kg = 2.508 x 1000 = 2508g]
C = ? (let unknown value be Z)
Φ = (Final temperature - Initial temperature)
= 42.061°C - 4.051°C
= 38.01°C
Apply the formula, Q = MCΦ
3420J = 2508g x Z x 38.01°C
3420J = 95329.08g•°C x Z
Z = (3420J / 95329.08g•°C)
Z = 0.03588 J/g°C
Round the value of Z to the nearest thousandth, hence Z = 0.036 J/g°C
Thus, the specific heat of the substance is 0.036 J/g°C
The number of moles of NaOh that are contained in 65ml of 2.20M solution NaOh in H2o is calculated using the below formula
moles = molarity x volume /1000
that is 65 x2.20 /1000= 0.143 moles
Answer:
Carbondioxide, water and ATP
Explanation:
The reaction is called aerobic respiration because oxygen from the air is needed for it to work.
Answer: a. Synthesis
Explanation:
a. Synthesis reaction is a chemical reaction in which two reactants are combining to form one product.
Example: 
Thus magnesium in its elemental form is combining with oxygen to form magnesium oxide.
b. Double displacement reaction is one in which exchange of ions take place.
Example: 
c. Decomposition is a type of chemical reaction in which one reactant gives two or more than two products.
Example: 
Explanation:
a. 0.0093
Number of significant figures = 2
All zero’s preceding the first integers are never significant
b. 120.9
Number of significant figures = 4
All zero’s between integers are always significant.
c. 1,000
Number of significant figures = 1
All zeroes used solely for spacing the decimal point are not significant.
d. 1.008
Number of significant figures = 4
All zero’s between integers are always significant.
All zero’s after the decimal point are always significant.
e. 670
Number of significant figures = 2
All zeroes used solely for spacing the decimal point are not significant.
f. 0.184
Number of significant figures = 3
All zero’s after the decimal point are always significant.
g. 1.30
Number of significant figures = 3
All zero’s after the decimal point are always significant.
