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At 1 atm, how much energy is required to heat 93.0 g of H2O(s) at –24.0 °C to H2O(g) at 115.0 °C?
 5 months ago
 5 months ago
At 1 atm, how much energy is required to heat 93.0 g of H2O(s) at –24.0 °C to H2O(g) at 115.0 °C?
 5 months ago
 5 months ago

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aaronqBest ResponseYou've already chosen the best response.2
you need to use 2 equations, in 5 steps. (1) \(q=H_{fusion/vap}*m\) (2) \(q=m*C_p*\Delta T\) dw:1382470856637:dw In A, your heating up the ice from 24 to 0 degrees: use equation (2) and the appropriate \(C_P\). In B, the ice is melting, use equation (1), use appropriate \(H_{fusion}\) In C, you're heating up the water form 0 to 100 degrees, use equation (2). Use appropriate \(C_p\). In D, you're vaporizing/boiling the water, use equation (1), use appropriate \(H_{vap}\). In E, you're heating up the water vapour/steam, use equation (2), use appropriate \(C_p\).
 5 months ago
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