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If the specific heat of water is ca increase the temperature of 75 g of water by 30 °C? 1gx1°C» how many calories of heat are needed to #calories Specific heat = (#gram x # degrees temperature changed)

If the specific heat of water is ca increase the temperature of 75 g of water by 30 °C? 1gx1°C» how many calories of heat are needed to #calories Specific heat = (#gram x # degrees temperature changed)

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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## Heat and Atomic Mass Calculation ### Specific Heat Calculation If the specific heat of water is \(1 \, \text{cal}/(\text{g} \cdot ^\circ \text{C})\), how many calories of heat are needed to increase the temperature of 75 g of water by 30 °C? #### Specific Heat Formula \[ \text{Specific heat} = \frac{\# \text{calories}}{(\# \text{grams} \times \# \text{degrees temperature changed})} \] ### Atomic and Molecular Masses One mole of atomic units (atoms, molecules, ions, electrons, etc.) is \(6.022 \times 10^{23}\) units (similar to how a dozen equals 12 items). The mass in grams of \(6.022 \times 10^{23}\) atoms of carbon is 12.00 grams or 1 mole, meaning 1 gram atomic mass of carbon atoms = 12.00 gram of carbon. We find the atomic masses for elements on the periodic table. #### Number of Moles of Atoms \[ \# \text{moles of atoms} = \frac{(\# \text{grams of atoms in sample})}{(\text{gram atomic mass})} \] #### Number of Moles of Molecules \[ \# \text{moles of molecules} = \frac{(\# \text{grams of molecules in sample})}{(\text{gram molecular mass})} \] ### Exercises #### 3. a. Calculate the mass of sulfur: \[ \text{3 gram atomic mass of sulfur atoms} = \_ \, \text{grams of sulfur}? \] #### 3. b. Calculate the mass in grams of \(6.022 \times 10^{23}\) molecules or a mole of sulfur dioxide (\(\text{SO}_2\)): \[ \text{SO}_2 = \left[32.07 \, \text{g} + (2 \times \_ \, \text{g})\right] \text{ or } \_ \, \text{grams}? \] ### Problem Sterling silver contains 92.5% silver and 7.5% copper. A sterling silver dish weighs 185.0 g. What mass of copper is in the dish? --- Feel free to go through each section
Transcribed Image Text:## Heat and Atomic Mass Calculation ### Specific Heat Calculation If the specific heat of water is \(1 \, \text{cal}/(\text{g} \cdot ^\circ \text{C})\), how many calories of heat are needed to increase the temperature of 75 g of water by 30 °C? #### Specific Heat Formula \[ \text{Specific heat} = \frac{\# \text{calories}}{(\# \text{grams} \times \# \text{degrees temperature changed})} \] ### Atomic and Molecular Masses One mole of atomic units (atoms, molecules, ions, electrons, etc.) is \(6.022 \times 10^{23}\) units (similar to how a dozen equals 12 items). The mass in grams of \(6.022 \times 10^{23}\) atoms of carbon is 12.00 grams or 1 mole, meaning 1 gram atomic mass of carbon atoms = 12.00 gram of carbon. We find the atomic masses for elements on the periodic table. #### Number of Moles of Atoms \[ \# \text{moles of atoms} = \frac{(\# \text{grams of atoms in sample})}{(\text{gram atomic mass})} \] #### Number of Moles of Molecules \[ \# \text{moles of molecules} = \frac{(\# \text{grams of molecules in sample})}{(\text{gram molecular mass})} \] ### Exercises #### 3. a. Calculate the mass of sulfur: \[ \text{3 gram atomic mass of sulfur atoms} = \_ \, \text{grams of sulfur}? \] #### 3. b. Calculate the mass in grams of \(6.022 \times 10^{23}\) molecules or a mole of sulfur dioxide (\(\text{SO}_2\)): \[ \text{SO}_2 = \left[32.07 \, \text{g} + (2 \times \_ \, \text{g})\right] \text{ or } \_ \, \text{grams}? \] ### Problem Sterling silver contains 92.5% silver and 7.5% copper. A sterling silver dish weighs 185.0 g. What mass of copper is in the dish? --- Feel free to go through each section
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