<span>Using proportions,
if x is the unknown volume we have:
1.84 / 1 = 42.5 / x </span>
<span>
Multiply both sides above by x:
1.84*x / 1 = 42.5
1.84*x = 42.5
Divide both sides by 1.84:
x = 42.5 / 1.84</span>
<span>X = 23.10 mL</span>
The specific heat capacity of unknown substance is 1.333 g/j/°c
<u><em> calculation</em></u>
Specific heat capacity is calculated using Q= MCΔT formula
where;
Q(heat)= 800 j
M(mass) = 30 g
C(specific heat capacity) =?
ΔT( change in temperature) = 40°c - 20°c = 20°c
make C the subject of the formula by diving both side of the formula by MΔT
C is therefore = Q/MΔT
800j / 30 g x 20°c = 1.333 j/g/°c
B and C are in excess so amount of E will be determined by A.
Amount of product is determined by limiting reagents - Always.
Hence 6 moles of E will be formed.
Hope this helps!
Answer:
Explanation:
Let final temperature be T .
vapor is at 102⁰C
loss of heat by vapor in turning into water at 100⁰C
= 2.6 x 2 x 1.996 + 2.6 x 2260 = 5886.37 J
loss of heat to lower temperature to T
2.6 x 4.186 x ( 100 - T )
1088.36 - 10.88 T
Total heat loss = 5886.37 + 1088.36 - 10.88 T
= 6974.73 - 10.88 T
heat gain by silver to gain temperature from 1⁰C to T⁰C
= 1250 x ( T - 1 ) x .235 = 293.75 T - 293.75
heat gain = heat loss
293.75 T - 293.75 = 6974.73 - 10.88 T
304.63 T = 7268.48
T = 23.86°C .
We are given initially with 1.2 x 1024 molecules of water, added further with <span>5.0 moles of water. we are asked to determine the total number of molecules of water after the addition. We just </span> convert the number of moles to number of molecules. 5 moles of water is equal to 3.011x 10^24 molecules. The total number is that we add the initial and the additional, equivalent to 4.211 x10^24 molecules.
