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An automobile tire was inflated to a pressure of 24 lb in-2 (1.00 atm = 14.7 lb in-2 ) on a winter’s day when the temperature was –5 o C. What pressure will be found assuming no leaks have occurred and that the volume is constant, on a subsequent summer’s day when the temperature is 35 o C? What complications should be taken into account in practice?
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Chemistry, 22.06.2019 00:30, natalie1755
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Chemistry, 22.06.2019 02:10, vapelordcarl69
When 225mg of anthracene, c14h10(s), was burned in a bomb calorimeter the temperature rose by 1.75k. calculate the calorimeter constant. by how much will the temperature rise when 125mg of phenol, c6h5oh(s), is burned in the calorimeter under the same conditions? (δch< (c14h10,s)=–7061 kj mol−1.)
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An automobile tire was inflated to a pressure of 24 lb in-2 (1.00 atm = 14.7 lb in-2 ) on a winter’s...
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