Based on the data, the increase in temperature of the methanol would be 413.0 \u00b0C<\/strong>.<\/p>\n\n\n\n The relationship between heat energy, mass, specific heat, and temperature change is described by the specific heat formula. This principle states that the amount of heat absorbed or released by a substance is directly proportional to its mass and the change in its temperature. The formula is expressed as:<\/p>\n\n\n\n Q = mc\u0394T<\/strong><\/p>\n\n\n\n Where:<\/p>\n\n\n\n Step 1: Determine the mass of the methanol.<\/strong> Step 2: Convert the heat energy to Joules.<\/strong> Step 3: Calculate the temperature increase (\u0394T).<\/strong> \u0394T = Q \/ (mc)<\/strong><\/p>\n\n\n\n Now, substitute the known values into the equation:<\/p>\n\n\n\n \u0394T = 836,000 J \/ (800 g \u00d7 2.53 J\/g\u00b0C) Therefore, the absorption of 836.0 kJ of heat would cause the temperature of 1.0 L of methanol to increase by 413.0 \u00b0C.thumb_upthumb_down<\/p>\n\n\n\n Suppose it is winter and the system is filled with methanol. The density of methanol is 0.80 g\/cm3. What would be the increase in temperature of the methanol if it absorbed 836.0 kJ of heat The Correct Answer and Explanation is: Based on the data, the increase in temperature of the methanol would be 413.0 \u00b0C. 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\n\n\n\nExplanation<\/h3>\n\n\n\n
\n
The problem does not provide the mass directly but gives the density. To make the problem solvable, we must assume a standard volume, such as 1.0 liter (1000 cm\u00b3). Using the density, we can calculate the mass.<\/p>\n\n\n\n\n
The heat absorbed (Q) is given in kilojoules (kJ). We must convert it to Joules to match the units of the specific heat capacity.<\/p>\n\n\n\n\n
Rearrange the specific heat formula to solve for \u0394T:<\/p>\n\n\n\n
\u0394T = 836,000 \/ 2024
\u0394T = 413.0 \u00b0C<\/strong><\/p>\n\n\n\n![\"\"](\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner4-887.jpeg\")
<\/figure>\n","protected":false},"excerpt":{"rendered":"